Aqueous Reactions

Open Ended

How do precipitation, acid-base, and redox reactions differ in their roles within aqueous solutions?

Multiple Choice

Why is water considered an effective solvent in many chemical reactions?

• Because it is a non-polar molecule

• Because it can dissolve only organic compounds

• Because it can dissolve a wide variety of substances due to its polarity

• Because it does not interact with other molecules

Multiple Choice

Which of the following best describes a solvent?

• A substance that is dissolved in a solution

• A homogenous mixture of two or more substances

• The dissolving medium, usually present in greater quantity

• A substance that cannot dissolve other substances

Open Ended

Explain the difference between an electrolyte and a nonelectrolyte based on their behavior in aqueous solution.

Multiple Choice

Which of the following statements about ionic compounds in water is/are correct?

• They dissociate into their component ions.

• They remain as whole molecules.

• They do not dissolve at all.

• They form covalent bonds with water.

Open Ended

According to the slides, what is the main difference in how molecular compounds and ionic compounds behave in water?

Multiple Choice

Which of the following is a strong electrolyte?

• C12H22O11 (sucrose)

• HCl (aq)

• NH3 (ammonia)

• H2C3O2 (acetic acid)

Open Ended

Weak acids are better conductors if they are dilute, as you will see in lab. Explain why this is the case based on the behavior of weak electrolytes in water.

Multiple Select

Which of the following statements about insoluble substances are correct?

• They have solubility less than 0.01 mol/L.

• Water molecules cannot overcome the attraction between the ions.

• They dissolve completely in water.

• They always contain alkali metals.

Multiple Choice

Which of the following best describes a precipitation reaction?

• A reaction that results in an insoluble product.

• A reaction that produces only gases.

• A reaction that forms only weak electrolytes.

• A reaction that always produces water.

Multiple Choice

What is the yellow solid formed when KI(aq) reacts with Pb(NO3)2(aq)?

• PbI2(s)

• KNO3(aq)

• KI(aq)

• Pb(NO3)2(aq)

Multiple Choice

Which of the following compounds is soluble in water with no important exceptions?

• NaNO3

• AgCl

• BaSO4

• CaCO3

Multiple Choice

Which of the following anions forms insoluble compounds with Ag+, Hg2^2+, and Pb2+?

• Cl-

• NO3-

• C2H3O2-

• SO4^2-

Multiple Choice

Which ions are exceptions to the insolubility of S2- compounds?

• NH4+ and Group 1 metals and Ba2+, Sr2+, Ca2+

• Ag+, Hg2^2+, Pb2+

• Group 1 metals and Ba2+, Sr2+, Ca2+

• None

Open Ended

Explain the difference between a complete ionic equation and a net ionic equation using the reaction between Pb(NO3)2 and KI.

Multiple Choice

Which of the following is another name for a double displacement reaction?

• Exchange reaction

• Decomposition reaction

• Redox reaction

• Combustion reaction

Multiple Select

Select all the correct steps involved in writing a net ionic equation.

• Write a balanced molecular equation.

• Rewrite the equation showing ions of strong electrolytes only.

• Identify and cancel all spectator ions.

• Balance the charges by adding electrons.

Multiple Choice

Which of the following statements best describes acids according to the information provided?

• Acids are substances that accept protons.

• Acids are substances that donate protons.

• Acids decrease the concentration of H+ ions in water.

• Acids are always solid at room temperature.

Open Ended

Compare monoprotic and diprotic acids in terms of their ionization process and the number of H+ ions released per molecule.

Multiple Choice

Which of the following statements about hydrofluoric acid (HF) is correct?

• HF is a strong acid and is not very reactive.

• HF is a weak acid but highly reactive due to the F- ion.

• HF can be stored in glass containers safely.

• HF is used to neutralize bases in the lab.

Multiple Select

Select all the correct statements about bases from the following:

• Bases increase the concentration of OH- ions in water.

• NH3 is a strong electrolyte.

• NH3 accepts an H+ ion from water.

• About 1% of NH3 ionizes to form NH4+/OH-.

Open Ended

Explain the difference between strong and weak acids and bases in terms of their ionization in solution.

Multiple Choice

Which metal is more reactive than calcium?

• magnesium
• potassium
• silver
• aluminum

Multiple Choice

During an oxidation-reduction reaction, the number of electrons gained is

• equal to the number of electrons lost

• equal to the number of protons gained

• less than the number of electrons lost

• less than the number of protons gained

Multiple Choice

When a sample of Mg(s) reacts completely with O₂(g), the Mg(s) loses 5.0 moles of electrons. How many moles of electrons are gained by the O₂(g)?

• 1.0 mol

• 2.5 mol

• 5.0 mol

• 10.0 mol

Multiple Choice

Identify the type of reaction shown.

• Single replacement

• Double replacement

• Synthesis

• Decomposition

Multiple Choice

2 MgI₂ + Mn(SO₃)₂ ----> 2 MgSO₃ + MnI₄

• Synthesis (or combination)
• Decomposition
• Single displacement
• Double displacement

Multiple Choice

What reaction is shown in this chemical equation?

• water being formed in the air

• fructose being made in a plant

• your body breaking down a carbohydrate

• baking soda and vinegar reaction

Open Ended

How do aqueous solutions facilitate different types of chemical reactions, and why is water considered an effective solvent in these processes?

Multiple Choice

What are the three major types of chemical processes that occur in aqueous solutions?

• Precipitation reactions, Acid-base reactions, Redox reactions

• Combustion reactions, Synthesis reactions, Decomposition reactions

• Single displacement, Double displacement, Combustion

• Neutralization, Polymerization, Decomposition